Complete combustion of $1.80 \, g$ of an oxygen-containing compound $(C_xH_yO_z)$ gave $2.64 \, g$ of $CO_2$ and $1.08 \, g$ of $H_2O$. The percentage of oxygen in the organic compound is

An organic compound gave the following results: $C = 53.3\%$,$H = 15.6\%$,$N = 31.1\%$. The molecular weight of the compound is $45$. What is the molecular formula of the compound?

The empirical formula of a compound is $CH_2$. If the molar mass of the compound is $42 \ g/mol$,what is its molecular formula?

On complete combustion of $0.492 \text{ g}$ of an organic compound containing $C$, $H$, and $O$, $0.7938 \text{ g}$ of $CO_2$ and $0.4428 \text{ g}$ of $H_2O$ were produced. The percentage composition of oxygen in the compound is $........$

$64 \, g$ of an organic compound contains $24 \, g$ of carbon,$8 \, g$ of hydrogen,and the rest oxygen. The empirical formula of the compound is

The empirical formula of a compound is $CH$. Its molecular weight is $78$. The molecular formula of the compound will be